For a $0.1 \ M$ aqueous pyridine solution,if the pyridinium ion concentration is produced such that the degree of dissociation is $0.013 \%$,calculate the concentration of the pyridinium ion.
- A$1.3 \times 10^{-5} \ M$
- B$1.3 \times 10^{-4} \ M$
- C$1.3 \times 10^{-3} \ M$
- D$1.3 \times 10^{-2} \ M$
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What is the $pH$ of $0.001 \,M$ aniline solution? The ionization constant of aniline can be taken from the table. Calculate the degree of ionization of aniline in the solution. Also,calculate the ionization constant of the conjugate acid of aniline.
Base $K_{b}$ Dimethylamine,$(CH_{3})_{2}NH$ $5.4 \times 10^{-4}$ Triethylamine,$(C_{2}H_{5})_{3}N$ $6.45 \times 10^{-5}$ Ammonia,$NH_{3}$ $1.77 \times 10^{-5}$ Quinine $1.10 \times 10^{-6}$ Pyridine,$C_{5}H_{5}N$ $1.77 \times 10^{-9}$ Aniline,$C_{6}H_{5}NH_{2}$ $4.27 \times 10^{-10}$ Urea,$CO(NH_{2})_{2}$ $1.3 \times 10^{-14}$
| Base | $K_{b}$ |
| Dimethylamine,$(CH_{3})_{2}NH$ | $5.4 \times 10^{-4}$ |
| Triethylamine,$(C_{2}H_{5})_{3}N$ | $6.45 \times 10^{-5}$ |
| Ammonia,$NH_{3}$ | $1.77 \times 10^{-5}$ |
| Quinine | $1.10 \times 10^{-6}$ |
| Pyridine,$C_{5}H_{5}N$ | $1.77 \times 10^{-9}$ |
| Aniline,$C_{6}H_{5}NH_{2}$ | $4.27 \times 10^{-10}$ |
| Urea,$CO(NH_{2})_{2}$ | $1.3 \times 10^{-14}$ |
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